Quantum number ml

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Maaria Abdel-Moneim 2I
Posts: 40
Joined: Wed Sep 30, 2020 10:09 pm

Quantum number ml

Postby Maaria Abdel-Moneim 2I » Fri Oct 23, 2020 1:39 pm

In Dr.Lavelle's lecture he talked about how the quantum number ml is like a range of values from +l to -l. I was wondering if it is a range how do we know which quantum number it actually is?

Annie Tong 2G
Posts: 36
Joined: Wed Sep 30, 2020 9:42 pm

Re: Quantum number ml

Postby Annie Tong 2G » Fri Oct 23, 2020 1:56 pm

Each magnetic quantum number refers to a specific orbital of a subshell. So unless it's specified, we don't know which quantum number it is.

Alen_Huang_3A
Posts: 39
Joined: Wed Sep 30, 2020 9:50 pm

Re: Quantum number ml

Postby Alen_Huang_3A » Fri Oct 23, 2020 2:42 pm

ml doesn't only range from -1 to 1, when l is 2 ml ranges from -2 to 2 cause when l = 2 we're talking about the d subshell which has 5 orbitals and -2 to 2 each represent one of those orbitals

Anthony_3C
Posts: 29
Joined: Wed Sep 30, 2020 10:00 pm

Re: Quantum number ml

Postby Anthony_3C » Sun Oct 25, 2020 8:14 pm

To clarify, the range only indicates the "possible values" of ml (orbitals) , which is based on the value of l. L indicates the subshells s, p, d, f etc., with l = 0 representing s, 1 representing p, and so on. It would be better to visualize this concept by looking at the periodic table. The final valence electron of H and He are both in n = 1, l = 0, ml = 0(1s). Li and Be are in n = 2, l = 0, ml = 0(2s). The final valence electron of B, C, N, O, F, Ne are all in the 2p subshell l but have different values for ml.
B and C are in ml = -1, N and O are in ml = 0, and F and Ne are in ml = 1. Note that there are two electrons in an orbital. You could observe from this pattern that the subshell s(l=0) has 1 orbital(ml=0), and the subshell p has 3 orbirtals(ml = -1,0,or1). Therefore d would have 5 orbitals, and f would have 7, and so on.

Hope this helps!!




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